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25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbonate solution. What is the volume of this HCl solution required to titrate 30 mL of 0.2 M aqueous NaOH solution?
- a)25 mL
- b)50 mL
- c)12.5 mL
- d)75 mL
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbona...
HCl with Na2CO3
Eq. of HCl = Eq. of Na2CO3
Eq of HCl = Eq. of NaOH
V = 25 ml
Eq. of HCl = Eq. of Na2CO3
Eq of HCl = Eq. of NaOH
V = 25 ml
Most Upvoted Answer
25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbona...
To determine the volume of the HCl solution required to titrate 30 mL of 0.2 M NaOH solution, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between HCl and NaOH.
The balanced chemical equation for the reaction is as follows:
HCl + NaOH → NaCl + H2O
From the equation, we can see that the stoichiometric ratio between HCl and NaOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of NaOH.
Given that 25 mL of the HCl solution requires 30 mL of 0.1 M sodium carbonate solution, we can use this information to determine the concentration of the HCl solution.
Step 1: Calculate the number of moles of sodium carbonate used:
Molarity (M) = moles (mol) / volume (L)
0.1 M = moles / 0.030 L
moles = 0.1 M × 0.030 L = 0.003 mol
Step 2: Use the stoichiometric ratio to determine the number of moles of HCl used:
Since the stoichiometric ratio between sodium carbonate and HCl is 1:2, the number of moles of HCl used is twice the number of moles of sodium carbonate used.
moles of HCl = 2 × 0.003 mol = 0.006 mol
Step 3: Calculate the concentration of the HCl solution:
Molarity (M) = moles (mol) / volume (L)
M = 0.006 mol / 0.025 L = 0.24 M
Now that we have determined the concentration of the HCl solution, we can use it to calculate the volume of HCl solution required to titrate 30 mL of 0.2 M NaOH solution.
Step 4: Use the stoichiometric ratio to calculate the volume of HCl solution:
Molarity (M) = moles (mol) / volume (L)
0.24 M = 0.006 mol / volume (L)
volume (L) = 0.006 mol / 0.24 M = 0.025 L = 25 mL
Therefore, the volume of the HCl solution required to titrate 30 mL of 0.2 M NaOH solution is 25 mL, which corresponds to option A.
The balanced chemical equation for the reaction is as follows:
HCl + NaOH → NaCl + H2O
From the equation, we can see that the stoichiometric ratio between HCl and NaOH is 1:1. This means that 1 mole of HCl reacts with 1 mole of NaOH.
Given that 25 mL of the HCl solution requires 30 mL of 0.1 M sodium carbonate solution, we can use this information to determine the concentration of the HCl solution.
Step 1: Calculate the number of moles of sodium carbonate used:
Molarity (M) = moles (mol) / volume (L)
0.1 M = moles / 0.030 L
moles = 0.1 M × 0.030 L = 0.003 mol
Step 2: Use the stoichiometric ratio to determine the number of moles of HCl used:
Since the stoichiometric ratio between sodium carbonate and HCl is 1:2, the number of moles of HCl used is twice the number of moles of sodium carbonate used.
moles of HCl = 2 × 0.003 mol = 0.006 mol
Step 3: Calculate the concentration of the HCl solution:
Molarity (M) = moles (mol) / volume (L)
M = 0.006 mol / 0.025 L = 0.24 M
Now that we have determined the concentration of the HCl solution, we can use it to calculate the volume of HCl solution required to titrate 30 mL of 0.2 M NaOH solution.
Step 4: Use the stoichiometric ratio to calculate the volume of HCl solution:
Molarity (M) = moles (mol) / volume (L)
0.24 M = 0.006 mol / volume (L)
volume (L) = 0.006 mol / 0.24 M = 0.025 L = 25 mL
Therefore, the volume of the HCl solution required to titrate 30 mL of 0.2 M NaOH solution is 25 mL, which corresponds to option A.
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25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbonate solution. What is the volume of this HCl solution required to titrate 30 mL of 0.2 M aqueous NaOH solution?a)25 mLb)50 mLc)12.5 mLd)75 mLCorrect answer is option 'A'. Can you explain this answer?
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25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbonate solution. What is the volume of this HCl solution required to titrate 30 mL of 0.2 M aqueous NaOH solution?a)25 mLb)50 mLc)12.5 mLd)75 mLCorrect answer is option 'A'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbonate solution. What is the volume of this HCl solution required to titrate 30 mL of 0.2 M aqueous NaOH solution?a)25 mLb)50 mLc)12.5 mLd)75 mLCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 25 ml of the given HCl solution requires 30 mL of 0.1 M sodium carbonate solution. What is the volume of this HCl solution required to titrate 30 mL of 0.2 M aqueous NaOH solution?a)25 mLb)50 mLc)12.5 mLd)75 mLCorrect answer is option 'A'. Can you explain this answer?.
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